3. Chemical Reactions

A metal (M) forms an oxide with the formula M2O. Identify the metal if the oxide is 16.99% O by mass.

A sample of an unknown compound was decomposed and found to be composed of 1.36 mol of oxygen, 4.10 mol of hydrogen, and 2.05 mol of carbon. What is the empirical formula of the unknown compound?

An unknown compound contains only carbon, hydrogen, and chlorine. Using combustion analysis, you burned 22.56 mg of the sample and collected 7.11 mg of H2O and 52.93 mg of CO2. What is the empirical formula of this compound?

An unknown compound contains only carbon, hydrogen, and oxygen. Using combustion analysis, you burned 19.31 mg of the sample and collected 17.96 mg of H2O and 43.89 mg of CO2. What is the empirical formula of this compound?

Determine the empirical formula of a compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen.

Which of the following methods can be used to determine the empirical formula of zinc oxide?

If 0.500 mol of copper combines with 0.250 mol of sulfur, what is the empirical formula of the copper sulfide product?

In an experiment, 10.0 g of sulfur and 10.0 g of oxygen react completely to form an oxide of sulfur. What is its empirical formula?

Upon combustion, a 0.8009 g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6004 g CO2 and 0.6551 g H2O. What is the empirical formula of the compound?

What is the empirical formula for a compound that contains 39.5% carbon, 2.21% hydrogen, and 58.3% chlorine?

What mass (in g) of carbon is in a sample of acetone (CH3COCH3) that contains 6.02 x 10^23 atoms of hydrogen?

What mass (in g) of carbon is in a sample of acetone (CH3COCH3) that contains 6.02 x 10^23 atoms of hydrogen?

A 4.386 g compound of hydrogen, carbon, and oxygen was burned in 9.389 g of oxygen, producing 6.184 g of carbon dioxide and 3.789 g of water. What is the empirical formula of the original sample?

A 48.3 g sample of an aluminum iodine compound contains 3.2 g of aluminum. What is the empirical formula for the compound?

What is the empirical formula for a compound containing 34.4% ethylenediamine, 2.101% Ni, 3.44% sulfate, and 60.06% water by mass?